Question

what is the balanced net ionic equation for the electrolysis of molten lithium fluoride? 2lif(l) → 2li(s) + f₂(g) 2li⁺(aq) + 2f⁻(aq) → 2li(s) + f₂(g) li⁺(aq) + f⁻(aq) → li(s) + f(l) lif(l) → li(s) + f(g)

Explanation:

1. First, recall the state of molten lithium fluoride: it's in liquid state (l), not aqueous (aq). So options with (aq) can be eliminated.
2. Then, consider the products of electrolysis of molten LiF: Li⁺ is reduced to Li(s), and F⁻ is oxidized. The oxidation of F⁻ produces F₂(g) (since F is a diatomic gas in elemental form), and the reaction must be balanced.
3. For the first option: \( 2\text{LiF}(l)

ightarrow 2\text{Li}(s) + \text{F}_2(g) \), let's check balancing. On the left, 2 Li and 2 F; on the right, 2 Li and 2 F (in F₂). The states are correct (molten LiF is l, Li is s, F₂ is g).

1. The fourth option has F(g) which is incorrect (F is diatomic as F₂). The second and third have aqueous ions which are wrong for molten salt.

Answer:

A. \( 2\text{LiF}(l)
ightarrow 2\text{Li}(s) + \text{F}_2(g) \)